Question 1

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 × 10-9

Accepted Answer

A)   1.4 × 10-3 M
B)   3.4 × 10-4 M
C)   8.7 × 10-4 M
D)   5.1 × 10-5 M
E)   -5 MF) B) and D)
G) A) and D)

Question 2

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. mL NaOH added 5.00 10.00 1.00 2.00
PH 6.98 7.46 7.93 10.31
What is the Ka for HClO?

Accepted Answer

A)   1.1 × 10-7
B)   3.5 × 10-8
C)   1.2 × 10-8
D)   4.9 × 10-11
E)   None of these choices are correct.F) A) and C)
G) B) and C)

Question 3

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10-8

Accepted Answer

A)   7.8 × 10-9 M
B)   1.8 × 10-8 M
C)   6.7 × 10-8 M
D)   1.6 × 10-7 M
E)   None of these choices are correct.F) C) and D)
G) A) and B)

Question 4

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Accepted Answer

A)   3(PO4) 2. 
A)     
B)     
C)     
D)     
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B)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
C)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of these choices are correct." class="answers-bank-image d-inline" rel="preload" >
D)   3(PO4) 2. 
A)     
B)     
C)     
D)     
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E)   None of these choices are correct.F) B) and C)
G) A) and E)

Question 5

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 × 10-12

Accepted Answer

A)   1.4 × 10-4 M
B)   3.4 × 10-5 M
C)   1.1 × 10-5 M
D)   1.6 × 10-6 M
E)   -6 MF) None of the above
G) B) and C)

Question 6

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Accepted Answer

A)   HOC6H4OCOOH, Ka = 1.0 × 10-3
B)   C6H4(COOH) 2, Ka = 2.9 × 10-4
C)   CH3COOH, Ka = 1.8 × 10-5
D)   C5H5O5COOH, Ka = 4.0 × 10-6
E)   HBrO, Ka = 2.3 × 10-9F) A) and C)
G) C) and D)

Question 7

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L-1)  with a strong base of the same concentration? -1)  with a strong base of the same concentration?   A)  A B)  B C)  C D)  D E)  E" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   A
B)   B
C)   C
D)   D
E)   EF) B) and E)
G) None of the above

Question 8

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO3) 2. Ksp = 6.5 × 10-6 for Ca(OH) 2) . Which of the following statements is correct?

Accepted Answer

A)   Calcium hydroxide precipitates until the solution is saturated.
B)   The solution is unsaturated and no precipitate forms.
C)   The concentration of calcium ions is reduced by the addition of the hydroxide ions.
D)   One must know Ksp for calcium nitrate to make meaningful predictions on this system.
E)   The presence of KOH will raise the solubility of Ca(NO3) 2.F) D) and E)
G) A) and B)

Question 9

Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 × 10-5)  is titrated with 0.05 M NaOH?

Accepted Answer

A)   bromphenol blue, pH range: 3.0-4.5
B)   bromcresol green, pH range: 3.8-5.4
C)   alizarin, pH range: 5.7-7.2
D)   phenol red, pH range: 6.9-8.2
E)   phenolphthalein, pH range: 8.0-10.1F) A) and B)
G) A) and C)

Question 10

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Accepted Answer

A) True 
 B)False

Question 11

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Accepted Answer

A)   increases
B)   decreases
C)   does not change
D)   first increases, then decreases
E)   first decreases, then increasesF) A) and B)
G) B) and D)

Question 12

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4) 2?

Accepted Answer

A)   6.5 × 10-12
B)   6.0 × 10-14
C)   5.2 × 10-24
D)   4.8 × 10-26
E)   1.0 × 10-26F) None of the above
G) A) and B)

Question 13

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10-4

Accepted Answer

A)   1.1 × 10-4 M
B)   2.6 × 10-4 M
C)   4.3 × 10-4 M
D)   6.7 × 10-5 M
E)   None of these choices are correct.F) B) and C)
G) B) and D)

Question 14

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO3) 3. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? Kf = 3.0 × 1033 for Al(OH) 4-

Accepted Answer

A)   1.8 × 10-7 M
B)   9.1 × 10-18 M
C)   1.0 × 10-31 M
D)   3.3 × 10-34 M
E)   7.1 × 10-36 MF) C) and D)
G) B) and C)

Question 15

For a diprotic acid H2A, the relationship Ka1 > Ka2 is always true.

Accepted Answer

A) True 
 B)False

Question 16

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3) 2 with 50.0 mL of 0.50 M Co(NO3) 2. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? Ksp = 2.2 × 10-20 for Cu(OH) 2, Ksp = 1.3 × 10-15 for Co(OH) 2

Accepted Answer

A)   Co(OH) 2; [OH-] = 6.9 × 10-6 M
B)   Co(OH)  2; [OH-] = 2.6 × 10-7 M
C)   Cu(OH)  2; [OH-] = 1.8 × 10-7 M
D)   Cu(OH)  2; [OH-] = 1.1 × 10-9 M
E)   Cu(OH)  2; [OH-] = 1.0 × 10-17 MF) None of the above
G) A) and C)

Question 17

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO-] = 0.5 M?

Accepted Answer

A)   The pH will increase slightly.
B)   The pH will increase significantly.
C)   The pH will decrease slightly.
D)   The pH will decrease significantly.
E)   Since it is a buffer solution, the pH will not be affected.F) B) and D)
G) B) and C)

Question 18

Calculate the solubility of barium carbonate, BaCO3, in pure water. Ksp = 2.0 × 10-9

Accepted Answer

A)   1.3 × 10-3 M
B)   3.2 × 10-5 M
C)   2.2 × 10-5 M
D)   4.5 × 10-5 M
E)   4.0 × 10-18 MF) C) and D)
G) B) and D)

Question 19

Which of the following aqueous mixtures would be a buffer system?

Accepted Answer

A)   HCl, NaCl
B)   HNO3, NaNO3
C)   H3PO4, H2PO4-
D)   H2SO4, CH3COOH
E)   NH3, NaOHF) C) and E)
G) A) and E)

Question 20

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 × 10-5

Accepted Answer

A)   4.49
B)   4.64
C)   4.85
D)   5.00
E)   5.52F) C) and D)
G) B) and C)

Exam 19: Ionic Equilibria in Aqueous Systems

Correct Answer
verified

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 × 10^-6 for Ca(OH) ₂) . Which of the following statements is correct?

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. mL NaOH added 5.00 10.00 1.00 2.00 PH 6.98 7.46 7.93 10.31 What is the Ka for HClO?

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 × 10^-5

Correct Answer
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The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO₃) ₃. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? K_f = 3.0 × 10³³ for Al(OH) ₄^-

Correct Answer
verified

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L^-1) with a strong base of the same concentration?

Correct Answer
verified

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10^-4

Correct Answer
verified

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Correct Answer
verified

Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 × 10^-12

Correct Answer
verified

For a diprotic acid H₂A, the relationship K_a1 > K_a2 is always true.

Correct Answer
verified

Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.05 M NaOH?

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

Which of the following aqueous mixtures would be a buffer system?

Correct Answer
verified

Calculate the solubility of barium carbonate, BaCO₃, in pure water. K_sp = 2.0 × 10^-9

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO^-] = 0.5 M?

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 × 10^-9

Correct Answer
verified

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10^-8

Correct Answer
verified

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

Correct AnswerverifiedShow Answer

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO3) 2. Ksp = 6.5 × 10-6 for Ca(OH) 2) . Which of the following statements is correct?

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. mL NaOH added 5.00 10.00 1.00 2.00 PH 6.98 7.46 7.93 10.31 What is the Ka for HClO?

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 × 10-5

Correct AnswerverifiedShow Answer

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO3) 3. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? Kf = 3.0 × 1033 for Al(OH) 4-

Correct AnswerverifiedShow Answer

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L-1) with a strong base of the same concentration?

Correct AnswerverifiedShow Answer

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10-4

Correct AnswerverifiedShow Answer

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Correct AnswerverifiedShow Answer

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 × 10-12

Correct AnswerverifiedShow Answer

For a diprotic acid H2A, the relationship Ka1 > Ka2 is always true.

Correct AnswerverifiedShow Answer

Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.05 M NaOH?

Correct AnswerverifiedShow Answer

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Correct AnswerverifiedShow Answer

Which of the following aqueous mixtures would be a buffer system?

Correct AnswerverifiedShow Answer

Calculate the solubility of barium carbonate, BaCO3, in pure water. Ksp = 2.0 × 10-9

Correct AnswerverifiedShow Answer

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO-] = 0.5 M?

Correct AnswerverifiedShow Answer

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 × 10-9

Correct AnswerverifiedShow Answer

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4) 2?

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10-8

Correct AnswerverifiedShow Answer

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct AnswerverifiedShow Answer

Correct Answer
verified

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 × 10^-6 for Ca(OH) ₂) . Which of the following statements is correct?

Correct Answer
verified

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 × 10^-5

Correct Answer
verified

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO₃) ₃. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? K_f = 3.0 × 10³³ for Al(OH) ₄^-

Correct Answer
verified

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak acid (0.10 mol L^-1) with a strong base of the same concentration?

Correct Answer
verified

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10^-4

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 × 10^-12

Correct Answer
verified

For a diprotic acid H₂A, the relationship K_a1 > K_a2 is always true.

Correct Answer
verified

Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.05 M NaOH?

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of barium carbonate, BaCO₃, in pure water. K_sp = 2.0 × 10^-9

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO^-] = 0.5 M?

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 × 10^-9

Correct Answer
verified

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10^-8

Correct Answer
verified

Correct Answer
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